Covalent bonding in Methane: CH 4 Carbon: 1S 2 2S 2 2P 2 Energy is released as carbon forms covalent bonds and the more energy released the more stable.

Slides:

Advertisements

Similar presentations

Word Splash – Write a few sentences about how the following terms are related.

Advertisements

Hybridization - The Blending of Orbitals Poodle + +Cocker Spaniel = = = = + +s orbitalp orbital Cockapoo sp orbital.

Hybridization - The Blending of Orbitals

Methane has 4 C-H sigma bonds. Four bonds of equal length. Bond vector separated by 109.5°. This angle also happens to be the angle that places.

Hybridisation of s and p orbitals in alkanes, alkenes and alkynes Unit 3.

Organic Compounds 11.2 The Tetrahedral Structure of Carbon 11.3 Polarity of Organic Molecules Chapter 11 Introduction to Organic Chemistry.

Hybridization Section Introduction A hybrid results from combining 2 of the same type of object and it has characteristics of both Atomic orbitals.

Ionic structure of Na + Cl - (s) This represents the maximum number of chloride ions that you can fit around a central sodium ion before the chloride ions.

© Prentice Hall 2001Chapter 11 Atomic Orbitals We cannot know the exact course of electrons as they orbit the nucleus - Heisenberg uncertainty principle.

Poodle + +Cocker Spaniel = = = = + +s orbitalp orbital Cockapoo sp orbital.

Covalent Bonding: orbitals. Hybridization - The Blending of Orbitals = = + +s orbitalp orbital sp orbital.

Molecular Shape Section 9.4

Methane, CH 4 less repulsion between the bonding pairs of electrons 109.5° 90°

Orbitalsand Covalent Bonds. Atomic Orbitals Don’t Work n to explain molecular geometry. n In methane, CH 4, the shape s tetrahedral. n The valence electrons.

COVALENT BONDING: ORBITALS HYBRIDIZATION (9.1). HYBRIDIZATION Consider methane,CH 4 C has 4 valence electrons 1s 2 2s 2 2p 2 This suggests that there.

Hybridization of Atomic Orbitals Some Material Copyright PGCC CHM 101 Sinex Some Graphics from Nelson Chemistry 12 Textbook.

Hybridization A Blending of Orbitals Methane CH 4 CH 4 Sometimes called “natural gas, ” methane is used to heat homes. Sometimes called “natural gas,

6-5 Molecular Geometry. VSEPR Theory VSEPR theory – states that repulsion between the sets of valence-level electrons surrounding an atom causes these.

Bonding theory Two methods of approximation are used to describe bonding between atoms. Valence bond method Bonds are assumed to be formed by overlap of.

Chapter 1: Structure and Bonding mcmurry. Coverage: 1. Electron Configurations. 2. Lewis Structures 3. Covalent and Ionic bonds 4. Atomic and Molecular.

SWBAT: Draw sp hybrid bonding orbitals for carbon

Lecture 2 Chemical Bonds: Atomic Orbital Theory and Molecular Orbital Theory Dr. A.K.M. Shafiqul Islam

HL Bonding Hybridisation. Hybridization is a model which is used to explain the behavior of atomic orbitals during the formation of covalent bonds. When.

Hybridization Polarity Intermolecular Forces SCH4U.

Hybridization Section Introduction A hybrid results from combining 2 of the same type of object and it has characteristics of both Atomic orbitals.

Molecular Orbitals. Organic compounds are organised into groups according to similarities and differences in their structure. Groups of atoms within a.

14.2 HYBRIDIZATION. ESSENTIAL IDEA Hybridization results from the mixing of atomic orbitals to form the same number of new equivalent hybrid orbitals.

Hybridization and Other Good Stuff. Introduction A hybrid results from combining two of the same type of objects, and it has characteristics of both Atomic.

Chapter 8 Lecture 8.5 Hybridization Section 8.3 Bonding Theories.

Orbital Hybridisation & VSEPR Learning Goals Students will be able to predict the hybridization in a variety of compounds using Lewis Structures & energy.

Bonding Theories Part 2: VSEPR Theory. Objectives Describe how VSEPR theory helps predict the shapes of molecules Describe how VSEPR theory helps predict.

Hydrocarbons - Alkenes L.O. To know how to name alkenes To know and understand how the structure of alkenes arises and the isomerism possible Homework:

Warm-up  Draw the following in VSEPR a) Butane b) Cyclopropane c) Dichloromethane d) 2-Bromopropane.

Bonding in methane The simplest alkane, methane, has the molecular formula CH 4. Justify that formula. Write the electronic configuration of carbon and.

COVALENT BONDING: ORBITALS Chapter 9. Hybridization The mixing of atomic orbitals to form special molecular orbitals for bonding. The atoms are responding.

4.6 Quantum Mechanics and Bonding: Hybridization.

Hybridization Carbon configuration Carbon in excited state can form 4 bonds.

Hybridization & Frontier Molecular Orbital Theory

18.2 Bonding in Methane and Orbital Hybridization

Hybrid Orbitals © Evan P. Silberstein, 2010.

Structure and Bonding in Organic Chemistry

Ch 9 – Covalent Bonding: Orbitals

Honors Chemistry Mrs. Coyle

Reactions of Alkenes Z E Z 1.7.3

Structure and Bonding in Organic Chemistry

Sigma () and Pi () Bonds

Bonding Theories Part 2: VSEPR Theory.

The Shapes of Molecules

HYBRIDIZATION SIGMA AND PI BONDS

Molecular Shapes Lewis structures physical properties VSEPR

Molecular Shapes and Hybrid Orbitals

Honors Chemistry Mrs. Coyle

Ch 9 – Covalent Bonding: Orbitals

18.2 Valence bond theory: hybridized orbitals and polyatomic molecules

Qantum Mechanics and Bonding Hybridization

8.3 Molecular Orbitals When two atoms combine, the molecular orbital model assumes that their atomic orbitals overlap to produce molecular orbitals,

Covalent Bonding: Orbitals

methane, CH4 less repulsion between the bonding pairs of electrons

Chemical formula and Lewis Structures Constitutional Isomers

Covalent Bonding - Orbitals

Hybridization - The Blending of Orbitals

Sigma () and Pi () Bonds

Qantum Mechanics and Bonding Hybridization

Covalent Bonding - Orbitals

Hybridization - The Blending of Orbitals

Orbital Hybridization

Hybridization College Chemistry.

Orbital Hybridization

Presentation transcript:

Covalent bonding in Methane: CH 4 Carbon: 1S 2 2S 2 2P 2 Energy is released as carbon forms covalent bonds and the more energy released the more stable the molecule. If the 2S electron is promoted to 2P then 4 unpaired electrons can be used in bonding:

In methane, all four C-H bonds are identical, so the electrons in the S and P orbitals rearrange themselves in a process called hybridization hybridization The SP 3 orbitals are tetrahedral in shape to avoid electron repulsion between orbitals and this defines the shape of CH 4 where it can bond with 4 hydrogen atoms. Bond angle 109 o

In ethane, C 2 H 6 there are 4 SP 3 orbitals for each carbon atom available for bonding; Three between C and H and the remaining one between C and C forming a sigma (s) bond:

Ethene, CH 2 CH 2 has a different bonding structure: Three of the 2S and 2P electrons are hydridized this time, to leave a 2P orbital. Then three SP 2 hybrids form: Before C=C bonding Bonds forming (molecular orbitals)